Exam (elaborations)
XI Chem New Chap 5 Thermodynamics 112 Profound HOTS Statements
- Course
- Institution
XI Chem New Chap 5 Thermodynamics 112 Profound HOTS Statements
[Show more]
Seller
Follow
Hkane
Reviews received
Content preview
XI_Chem_New Chap-5_Thermodynamics_[True or False Statement Questions]Sl # Profound Statements [HOTS _ Thermodynamics] TRUE/FALSE
A negative ∆G indicates a spontaneous process; a positive ∆G indicates a non-spontaneous process.
1
2 Adiabatic conditions for a process require heat exchange (q ≠ 0).
3 Adiabatic conditions for a process require that there is no heat exchange (q = 0).
Enthalpy change alone determines the direction of spontaneity; entropy changes are irrelevant.
4
Enthalpy change alone does not determine the direction of spontaneity; entropy change is equally
5
important, as indicated by the Gibbs equation.
Enthalpy change alone does not determine the direction of spontaneity; entropy changes play a
6
significant role.
Enthalpy change for a chemical reaction in the gaseous state can be calculated using bond
7
enthalpies of reactants and products.
Enthalpy change for a chemical reaction in the gaseous state cannot be calculated using bond
8
enthalpies of reactants and products.
Enthalpy change for a reaction can be calculated using the heat capacity of a calorimeter,
9
temperature change, and reaction heat.
Enthalpy change for a reaction cannot be calculated using the heat capacity of a calorimeter,
10
temperature change, and reaction heat.
Enthalpy change for a reaction involving gases at constant pressure can be related to ΔU by
11
accounting for the pressure-volume work, ΔngRT.
Enthalpy change for a reaction involving gases at constant pressure cannot be related to ΔU by
12
accounting for the pressure-volume work, ΔngRT.
Enthalpy change is a measure of heat absorbed or evolved during a reaction. A negative ΔH
13
indicates heat release, while a positive ΔH indicates heat absorption.
Enthalpy change is a measure of work done during a reaction, with negative ΔH indicating work
14
input and positive ΔH indicating work output.
Enthalpy change is related to heat exchange in a reaction, with negative ΔrH indicating exothermic
15
reactions and positive ΔrH indicating endothermic reactions.
Enthalpy change is unrelated to heat exchange in a reaction, with negative ΔrH indicating
16
endothermic reactions and positive ΔrH indicating exothermic reactions.
17 Enthalpy change is useful for industrial processes and equilibrium constant calculations.
18 Enthalpy change is useless for industrial processes and equilibrium constant calculations.
Enthalpy is an extensive quantity, and its value depends on how the chemical equation is balanced.
19
Enthalpy is an intensive quantity, and its value depends on how the chemical equation is balanced.
20
Enthalpy of atomization is the enthalpy change when one mole of a substance in the gaseous state
21
is formed from its constituent atoms in their non-standard states.
Enthalpy of atomization is the enthalpy change when one mole of a substance in the gaseous state
22
is formed from its constituent atoms in their standard states.
Enthalpy of dilution refers to the enthalpy change when a solute is added to a solvent to create a
23
solution with lower concentrations.
Enthalpy of hydration: Change when gaseous ions dissolve in water, forming hydrated ions; crucial
24
for solubility and solution behavior.
Enthalpy of solution is change when a mole of substance dissolves in solvent; influenced by lattice
25
enthalpy and ion hydration.
Enthalpy of solution is change when a mole of substance precipitates from solvent; influenced by
26
lattice enthalpy and ion dehydration.
Enthalpy of solution: Change when a mole of substance dissolves in solvent; influenced by lattice
27
enthalpy and ion hydration.
1 OF 5 RI_Best Wishes
, XI_Chem_New Chap-5_Thermodynamics_[True or False Statement Questions]
Sl #Profound Statements [HOTS _ Thermodynamics] TRUE/FALSE
Enthalpy of solution: Change when a mole of substance precipitates from solvent; influenced by
28
lattice enthalpy and ion dehydration.
Entropy is a measure of disorder and randomness in a system. Spontaneous processes tend to
29
increase the overall entropy of a system and its surroundings.
Equilibrium constant (K) has no relation to standard Gibbs energy change (ΔG°), and ∆G° ≠ -RT ln K.
30
31 Equilibrium constant (K) relates to standard Gibbs energy change (ΔG°) as ΔG° = -RT ln K.
Estimating ΔG° from ΔH° and ΔS°, or direct K measurement enables calculating equilibrium
32
constants at different temperatures.
Estimating ΔG° from ΔH° and ΔS°, or direct K measurement, prevents calculating equilibrium
33
constants at different temperatures.
Exothermic reactions tend to be spontaneous as they release heat, increasing the disorder of the
34
surroundings and leading to positive entropy change.
For a spontaneous reaction, the change in Gibbs free energy (∆G) must be negative, reflecting the
35
balance between enthalpy and entropy changes.
For a spontaneous reaction, the change in Gibbs free energy (∆G) must be positive, reflecting the
36
imbalance between enthalpy and entropy changes.
37 For endothermic reactions, large positive ΔH leads to small K and limited product formation.
Gibbs energy provides a criterion for spontaneity at constant temperature and pressure. Negative
38
ΔG indicates a spontaneous process.
Gibbs energy provides no criterion for spontaneity at constant temperature and pressure. Negative
39
ΔG indicates a non-spontaneous process.
Gibbs free energy change (ΔG) accounts for both enthalpy (ΔH) and entropy (ΔS) changes,
40
determining spontaneity at constant temperature and pressure.
Gibbs free energy change (ΔG) ignores both enthalpy (ΔH) and entropy (ΔS) changes, providing no
41
information about spontaneity at constant temperature and pressure.
Heat of reaction at constant pressure, ∆H = qP, can be positive (endothermic) or negative
42
(exothermic) depending on heat absorption or release.
Heat of reaction at constant pressure, ∆H = qP, is always negative (exothermic) regardless of heat
43
absorption or release.
Internal energy change ΔU = q + w in a closed system: ΔU = change in energy, q = added heat, w =
44
work done.
Mean bond enthalpy represents the energy required to break a bond in a polyatomic molecule like
45
methane.
Mean bond enthalpy represents the energy required to create a bond in a polyatomic molecule
46
like methane.
Negative Gibbs energy (∆G) indicates non-spontaneous processes, where energy available for
47
useful work is less than system energy.
Negative Gibbs energy (∆G) indicates spontaneous processes, where energy available for useful
48
work exceeds system energy.
49
Positive ∆G implies non-spontaneity, requiring external energy input for the process to proceed.
Positive ∆G implies spontaneity, requiring no external energy input for the process to proceed.
50
Reversible processes proceed infinitely quickly through a series of non-equilibrium states, creating
51
constant disequilibrium between the system and surroundings.
Reversible processes proceed infinitely slowly through a series of equilibrium states, maintaining
52
near-equilibrium between the system and surroundings.
53 Spontaneity involves irreversible changes and doesn't naturally reverse direction.
2 OF 5 RI_Best Wishes
The benefits of buying summaries with Stuvia:
Guaranteed quality through customer reviews
Stuvia customers have reviewed more than 700,000 summaries. This how you know that you are buying the best documents.
Quick and easy check-out
You can quickly pay through credit card or Stuvia-credit for the summaries. There is no membership needed.
Focus on what matters
Your fellow students write the study notes themselves, which is why the documents are always reliable and up-to-date. This ensures you quickly get to the core!
Frequently asked questions
What do I get when I buy this document?
You get a PDF, available immediately after your purchase. The purchased document is accessible anytime, anywhere and indefinitely through your profile.
Satisfaction guarantee: how does it work?
Our satisfaction guarantee ensures that you always find a study document that suits you well. You fill out a form, and our customer service team takes care of the rest.
Who am I buying these notes from?
Stuvia is a marketplace, so you are not buying this document from us, but from seller Hkane. Stuvia facilitates payment to the seller.
Will I be stuck with a subscription?
No, you only buy these notes for $7.99. You're not tied to anything after your purchase.
Can Stuvia be trusted?
4.6 stars on Google & Trustpilot (+1000 reviews)
75323 documents were sold in the last 30 days
Founded in 2010, the go-to place to buy study notes for 14 years now